CHEM1102 Chemistry Model Assignment

1. Which one of the compounds A - E is a primary alcohol?

2. Which one of the compounds A - E will react with NaOH in an acid-base reaction?

3. Which one of the compounds A - E will react with HCl to form a quaternary ammonium salt?

4. Which one of the compounds A - E will react with dimethylamine, (CH3)2NH, to give an amide?

5. Which one of the compounds A - E will form a carboxylic acid upon treatment with acidified Na2Cr2O7 solution?

6. Which one of the following is the most stable carbocation? 

For questions 7 - 11, choose from A - E the term that best describes the relationship  between each of the following pairs of compounds. 

A. Conformational Isomers B. Constitutional Isomers C. Enantiomers D. Diastereomers E. Identical Compounds

12. Which one of compounds A - E can react with HCl in an electrophilic addition reaction?

13. Which one of compounds A - E will be formed upon the oxidation of 2-butanol?

14. Which one of compounds A - E will react with NaBH4  followed by aqueous acid to give a primary alcohol? 

15. Which one of compounds A - E undergoes an elimination reaction on treatment with hot alcoholic potassium hydroxide solution

16. Which one of compounds A - E is an example of a conjugated molecule? 

17. Which one of compounds A - E will form  

2-methyl-2-bromobutane upon treatment with HBr? 

18. Rank the following series of atoms in order of INCREASING electronegativity. N O F P As 

A N < O>

B F < O>

C As < P>

D As < P>

E F < N>

19. Which one of the following combinations does the titration curve represent? 

A Addition of a strong base to a weak acid 

B Addition of a weak base to a strong acid 

C Addition of a weak acid to a strong base 

D Addition of a strong acid to a strong base 

E Addition of a strong acid to a weak base

20. What is the value of the pKa that can be obtained from this titration curve? 

A 11.3 

B 10.0 

C 9.3 

D 5.3 

E 1.8

21. Which intermolecular forces are present in phenol, C6H5OH(s)? 

A London dispersion only 

B Dipole-dipole only 

C Hydrogen-bonding only 

D London dispersion and dipole-dipole 

E London dispersion, dipole-dipole and hydrogen bonding

22. A catalyst speeds up a chemical reaction by 

A changing the stoichiometry. 

B increasing the activation energy. 

C providing an alternative reaction mechanism of lower activation energy. 

D shifting the equilibrium towards the side of the product(s). 

E increasing the reaction enthalpy.

23. Which of the following gases can be liquefied at 25 °C?  

Gas          Critical point 

CH3Cl      144 °C, 66 atm 

SO2        158 °C, 78 atm 

CH4        –82 °C, 46 atm 

A SO2 only 

B CH4 only 

C CH3Cl and SO2 

D all of them 

E none of them

24. A solid has a very high melting point, is very hard, and its liquid is non conducting. The compound is 

A a discrete molecular solid. 

B a metallic solid. 

C a covalent network solid. 

D an ionic solid. 

E an amorphous solid.

25. When one mole of ice melts to liquid at 0 °C, 

A the entropy of the system decreases. 

B the entropy of the system remains the same. 

C the entropy of the system increases. 

D the order of the system increases. 

E None of the above

26. The entropy of a chemical system will usually increase when 

A a molecule is broken down into two or more smaller fragments.

B a reaction occurs that results in an increase in the moles of gas. 

C a solid changes to a liquid. 

D a liquid changes into a gas. 

E All of the above

27. Arrange the common unit cells of metals from the least dense packing to the most  dense packing. 

A body-centred cubic < face>

B body-centred cubic < simple>

C face-centred cubic < simple>

D simple cubic < body-centred cubic < face>

E simple cubic < face>

28. How many atoms are there in the face-centred cubic unit cell of iron? 

A # atoms = 18 (8) = 1 

B # atoms = 1 + 18 (8) = 2 

C # atoms = 12 (6) = 3 

D # atoms = 12 (6) + 18 (8) = 4 

E # atoms = 1 + 12 (6) + 18 (8) = 5

29. The normal boiling point of a liquid is 

A the only temperature at which there can be equilibrium between the liquid  and gas states. 

B the temperature above which the substance cannot exist as a liquid regardless  of the pressure. 

C the temperature at which the entropy of the liquid is equal to zero. 

D the temperature at which the vapour pressure of the liquid equals the ambient  atmospheric pressure. 

E the temperature at which the vapour pressure of the liquid equals 1 atm.

30. What is the geometry of the [Cr(OH2)6]3+ ion? 

A tetrahedral 

B trigonal bipyramidal 

C square planar 

D octahedral 

E linea

31. What is the ground state electronic configuration of Fe3+? 

A [Ar] 3s2 3p6 

B [Ar] 4s2 3d4 

C [Ar] 4s2 3d3 

D [Ar] 4s0 3d8 4p2 

E [Ar] 4s0 3d5

32. Which of the following species exist as isomers? 

[Co(NH3)6]3+, [PtCl2(NH3)2], Co(OH2)6Cl3, [Co(OH2)6]2+, [CdI4]2– 

A [PtCl2(NH3)2] and [Co(OH2)6]Cl3 

B [PtCl2(NH3)2] only 

C [CdI4]2– only 

D [Co(NH3)6]3+ and [Co(OH2)6]2+ 

E [Co(OH2)6]Cl3 and [Co(OH2)6]2+

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